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- https://chem.libretexts.org/Courses/Fullerton_College/Introductory_Chemistry_for_Allied_Health_(Chan)/19%3A_Acids_and_Bases/19.08%3A_BuffersA buffer is a solution that resists sudden changes in pH.
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Qualitative_Analysis_of_Common_Cations_in_Water_(Malik)/1%3A_Chemical_Principles/1.4%3A_pH_BuffersA pH buffer is an aqueous solution consisting of a weak acid and its conjugate base or vice versa, which minimizes pH change when a small amount of a strong acid or a strong base is added to it.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/ChemPRIME_(Moore_et_al.)/14%3A_Ionic_Equilibria_in_Aqueous_Solutions/14.08%3A_Buffer_SolutionsBuffers allow chemists to maintain a specific pH range for a reaction. Buffers utilize conjugate acid-base pairs to function. Read on to learn more about the specifics and calculations of buffers.
- https://chem.libretexts.org/Courses/Widener_University/CHEM_176%3A_General_Chemistry_II_(Fischer-Drowos)/05%3A_Acid-Base_Equilibria/5.07%3A_BuffersA solution containing a mixture of an acid and its conjugate base, or of a base and its conjugate acid, is called a buffer solution. Unlike in the case of an acid, base, or salt solution, the hydroniu...A solution containing a mixture of an acid and its conjugate base, or of a base and its conjugate acid, is called a buffer solution. Unlike in the case of an acid, base, or salt solution, the hydronium ion concentration of a buffer solution does not change greatly when a small amount of acid or base is added to the buffer solution. The base (or acid) in the buffer reacts with the added acid (or base).
- https://chem.libretexts.org/Ancillary_Materials/Worksheets/Worksheets%3A_Analytical_Chemistry_II/BuffersDetermine if each of the following results in the formation of a buffer solution. A solution prepared by mixing 10.00 mL of 0.100 M NaHCO 3 and 10.00 mL of 0.200 M Na 2 CO 3 . A solution prepared by m...Determine if each of the following results in the formation of a buffer solution. A solution prepared by mixing 10.00 mL of 0.100 M NaHCO 3 and 10.00 mL of 0.200 M Na 2 CO 3 . A solution prepared by mixing 25.00 mL of 0.50 M citric acid with 75.00 mL of 0.50 M NaOH. Describe how you would prepare 250 mL of a 100 mM acetate buffer with a pH of 5.0. You have the following available to you in the lab: 17.4 M acetic acid, solid sodium acetate, 1.0 M NaOH, and 1.0 M HCl.
- https://chem.libretexts.org/Courses/Oregon_Institute_of_Technology/OIT%3A_CHE_331_-_Organic_Chemistry_(Lund)/09%3A_Introduction_to_Acid-base_Reactions/9.02%3A_The_Acidity_ConstantYou are no doubt aware that some acids are stronger than others. The relative acidity of different compounds or functional groups – in other words, their relative capacity to donate a proton to a comm...You are no doubt aware that some acids are stronger than others. The relative acidity of different compounds or functional groups – in other words, their relative capacity to donate a proton to a common base under identical conditions – is quantified by a number called the acidity constant, abbreviated K
- https://chem.libretexts.org/Courses/Smith_College/CHM_222_Chemistry_II%3A_Organic_Chemistry_(2025)/11%3A_Carboxylic_Acids_and_Nitriles/11.04%3A_Biological_Acids_and_the_Henderson-Hasselbalch_Equation_(reference_only)use the Henderson-Hasselbalch equation to calculate the percentages of dissociated and undissociated acids [A − ] and [HA] in a solution, given the pK a value of the acid and the pH of the solution. A...use the Henderson-Hasselbalch equation to calculate the percentages of dissociated and undissociated acids [A − ] and [HA] in a solution, given the pK a value of the acid and the pH of the solution. Also, the Henderson-Hasselbalch allows for the pH of the solution to be calculated when the pK a of the acid is known along with the concentrations of the carboxylic acid and carboxylate are known.
- https://chem.libretexts.org/Courses/Stanford_Online_High_School/TEN2A-Acids/03%3A_Buffers/3.01%3A_Buffered_SolutionsBuffers are solutions that resist a change in pH after adding an acid or a base. Buffers contain a weak acid (\(HA\)) and its conjugate weak base (\(A^−\)). Adding a strong electrolyte that contains o...Buffers are solutions that resist a change in pH after adding an acid or a base. Buffers contain a weak acid (\(HA\)) and its conjugate weak base (\(A^−\)). Adding a strong electrolyte that contains one ion in common with a reaction system that is at equilibrium shifts the equilibrium in such a way as to reduce the concentration of the common ion. Buffers are characterized by their pH range and buffer capacity.
- https://chem.libretexts.org/Courses/Oregon_Institute_of_Technology/OIT%3A_CHE_332_--_Organic_Chemistry_II_(Lund)/7%3A_Acid-base_Reactions/7.2%3A_The_Acidity_ConstantYou are no doubt aware that some acids are stronger than others. The relative acidity of different compounds or functional groups – in other words, their relative capacity to donate a proton to a comm...You are no doubt aware that some acids are stronger than others. The relative acidity of different compounds or functional groups – in other words, their relative capacity to donate a proton to a common base under identical conditions – is quantified by a number called the acidity constant, abbreviated K
- https://chem.libretexts.org/Courses/University_of_Minnesota_Rochester/genchem2/2%3A_Acid-Base_Equilibria/2.6%3A_BuffersA solution containing a mixture of an acid and its conjugate base, or of a base and its conjugate acid, is called a buffer solution. Unlike in the case of an acid, base, or salt solution, the hydroniu...A solution containing a mixture of an acid and its conjugate base, or of a base and its conjugate acid, is called a buffer solution. Unlike in the case of an acid, base, or salt solution, the hydronium ion concentration of a buffer solution does not change greatly when a small amount of acid or base is added to the buffer solution. The base (or acid) in the buffer reacts with the added acid (or base).
- https://chem.libretexts.org/Courses/Los_Angeles_Trade_Technical_College/Analytical_Chemistry/2%3A_Analytical_Chemistry_2.0_(Harvey)/07%3A_Equilibrium_Chemistry/7.08%3A_Buffer_SolutionsAs outlined below, the Henderson–Hasselbalch approximation provides a simple way to calculate the pH of a buffer, and to determine the change in pH upon adding a strong acid or strong base.
